Differentiate strong and weak electrolytes.

An electrolyte is a substance that, when dissolved in water, produces a solution that can conduct electricity. The ability to conduct electricity is due to the presence of ions in these solutions.

Strong electrolytes are substances that dissociate completely into ions when dissolved in water. This results in a high concentration of ions in the solution and therefore, a high electrical conductivity. Weak electrolytes, on the other hand, partially dissociate into ions in water. This means that they only produce a small concentration of ions, resulting in lower electrical conductivity compared to strong electrolytes.

Strong electrolytes mainly include soluble salts, strong acids, and strong bases. Some examples of strong electrolytes are: 1. Sodium chloride (NaCl) 2. Potassium nitrate (KNO_3) 3. Hydrochloric acid (HCl) 4. Sulfuric acid (H_2SO_4) 5. Sodium hydroxide (NaOH) When these compounds dissolve in water, they dissociate completely into their constituent ions, leading to a high electrical conductivity of the solution.

Weak electrolytes comprise mainly weak acids and weak bases, and some slightly soluble salts. Some examples of weak electrolytes are: 1. Acetic acid (CH_3COOH) 2. Ammonium hydroxide (NH_4OH) 3. Carbonic acid (H_2CO_3) 4. Hydrogen fluoride (HF) These substances only partially dissociate into ions in water, resulting in a lower concentration of ions in the solution and lower electrical conductivity compared to strong electrolytes. In conclusion, the key difference between strong and weak electrolytes lies in the extent of ionization in water. Strong electrolytes dissociate completely into ions and exhibit high electrical conductivity, while weak electrolytes partially dissociate, producing a smaller concentration of ions and lower electrical conductivity.